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Q. No.Match List-I with List-II:
Choose the correct answer from the options given below:
| List-I (Order of reaction) | List-II (Unit of rate constant) | ||
| A. | Zero order | I. | \(\mathrm{mol}^{-1} \mathrm{~L} \mathrm{~s}^{-1}\) |
| B. | First order | II. | \(\mathrm{mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}\) |
| C. | Second order | III. | \(\mathrm {s}^{-1}\) |
| D. | Third order | IV. | \(\mathrm{mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) |
Choose the correct answer from the options given below:
| 1. | A-IV, B-III, C-II, D-I |
| 2. | A-I, B-II, C-III, D-IV |
| 3. | A-IV, B-III, C-I, D-II |
| 4. | A-IV, B-II, C-I, D-III |
Subtopic: Definition, Rate Constant, Rate Law | First Order Reaction Kinetics |
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Level 2: 60%+
NEET - 2026
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For a certain reaction R → Product, the plot of concentration [R] vs time has a negative slope as shown. The order of reaction is :
1. 0
2. 1
3. 2
4. 2.5
1. 0
2. 1
3. 2
4. 2.5
Subtopic: Definition, Rate Constant, Rate Law | Order, Molecularity and Mechanism |
68%
Level 2: 60%+
NEET - 2026
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Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T(K).
\(\ln k = 14\cdot34 - \frac{1\cdot25 \times 10^4}{T}\)
The energy of activation in kcal mol-1 for the reaction is :
(Given : k in \(s^{-1}, R = 1.987 ~\text{cal mol}^{-1} K^{-1})\)
1. 12.42
2. 14.34
3. 18.63
4. 24.84
\(\ln k = 14\cdot34 - \frac{1\cdot25 \times 10^4}{T}\)
The energy of activation in kcal mol-1 for the reaction is :
(Given : k in \(s^{-1}, R = 1.987 ~\text{cal mol}^{-1} K^{-1})\)
1. 12.42
2. 14.34
3. 18.63
4. 24.84
Subtopic: First Order Reaction Kinetics | Arrhenius Equation |
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Level 2: 60%+
NEET - 2026
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If the rate constant of a reaction is \(0.03 s^{-1}\), how much time does it take for \(7.2\text { mol L}^{-1}\) concentration of the reactant to get reduced to \(0.9~\text {mol L} ^{-1}?\)
(Given: log 2=0.301)
1. 210 s
2. 21.0 s
3. 69.3 s
4. 23.1 s
(Given: log 2=0.301)
1. 210 s
2. 21.0 s
3. 69.3 s
4. 23.1 s
Subtopic: First Order Reaction Kinetics |
64%
Level 2: 60%+
NEET - 2025
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\(C(s) + 2 H_2(g) \rightarrow CH_4(g); \Delta H = -74.8~kJ mol^{-1}\)
Which of the following diagrams gives an accurate representation of the above reaction?
[R→reactants; P→products]
Which of the following diagrams gives an accurate representation of the above reaction?
[R→reactants; P→products]
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
59%
Level 3: 35%-60%
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If the half-life \((t_{1/2})\) for a first order reaction is \(1~\text{minute}\), then the time required for \(99.9 \%\) completion of the reaction is closest to :
1. \(5~\text{minutes}\)
2. \(10~\text{minutes}\)
3. \(2~\text{minutes}\)
4. \(4~\text{minutes}\)
1. \(5~\text{minutes}\)
2. \(10~\text{minutes}\)
3. \(2~\text{minutes}\)
4. \(4~\text{minutes}\)
Subtopic: First Order Reaction Kinetics |
66%
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Activation energy of any chemical reaction can be calculated if one knows the value of:
| 1. | Probability of collision. |
| 2. | Orientation of reactant molecules during collision. |
| 3. | Rate constant at two different temperatures. |
| 4. | Rate constant at standard temperature. |
Subtopic: Arrhenius Equation |
69%
Level 2: 60%+
NEET - 2024
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Which plot of In k vs \(\frac{\text{I}}{\text{T}}\) is consistent with Arrhenius equation?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
68%
Level 2: 60%+
NEET - 2024
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The rate of a reaction quadruples when temperature changes from 27°C to 57°C. Calculate the energy of activation.
Given R = 8.314 J K–1 mol–1, log 4 = 0.6021
Given R = 8.314 J K–1 mol–1, log 4 = 0.6021
| 1. | 380.4 kJ/mol | 2. | 3.80 kJ/mol |
| 3. | 3804 kJ/mol | 4. | 38.04 kJ/mol |
Subtopic: Arrhenius Equation |
56%
Level 3: 35%-60%
NEET - 2024
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Which of the following expression is correct for the reaction given below?
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
| 1. | \(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 2. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\) |
| 3. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 4. | \( \dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\) |
Subtopic: Definition, Rate Constant, Rate Law |
89%
Level 1: 80%+
NEET - 2024
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